3. part B & C

Learning Goal: To use the Arrienius equation to calculate the activation energy. Calculate the value of ln(k2k1) where k1 and k2 correspond to the rate conctants at the As temperature rises, the average kinetic energy of initial and the final temperatures as defined in part A. molecules increases. In a chemical reaction, this: means that a higher percentage of the molecules possess the required activation energy, and the reaction goes laster. This relationship is shown by the Arrhenius equation k=AeE2/RT Where k is the rate constant, A is the frequency factor, Ea is the activation energy. R=8.3145 J/(K - mol) is the gas constant, and T is the Kelvin temperature. The following rearranged version of the equation is also usoful: ln(k2k1)=(RE2)(T21T11) Express your answer numerically. What is the activation energy of the reaction? Express your answer numerically in kilojoules per mole. The rate constant of a chemical reaction increased from 0.100s1 to 3,10s1 upon raising the temperature from 25.0C to 49.0C. Learning Goal: To use the Armenius equation to calculate the activation energy. Part A As temperature tises, the average kinetic energy of molecules increases. In a chemical reaction, this means that a higher percentage of the molecules possess the required activation energy, and the reaction. goes faster. This relationship is shown by the Armenius equation k=AeR/RT where k is the rate constant, A is the frequency factor, Ea is the activation energy, R=8.3145 J/(K+mol) is the gas constant, and T is the Kelvin temperature. The following rearranged version of the equation is also useful: ln(k2k1)=(REa)(T21T11) where k1 is the rate constant at temperature. T1. and k2 is the rate constant at temperature T2